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25 Cards in this Set
- Front
- Back
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What does Boyle's Law show, and what is the formula to demonstrate this relationship?
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the pressure-volume relationship
volume is inversely proportional to pressure V= constant x 1/P P1V1=P2V2 |
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What is Charles's Law, and what formula is used to represent this relationship?
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relationship between pressure and volume
volume of a gas is directly proportional to the absolute temperature V= constant x T V1/T1 = V2/T2 |
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What is Avogadro's Law and what formula is used to describe it?
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quantity-volume relationship
volume of a gas is directly proportional to the number of mules of gas V = constant x n |
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What is the ideal gas equation, and where does this equation come from?
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PV=nRT
combination of Boyle's Law, Charles's Law, and Avogadro's Law an ideal gas exactly follows the equation |
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What is Dalton's Law of Partial Pressures?
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the total pressure of a mixture of gases is the sum of the individual gas pressures
Pt= P1+P2+P3+... |
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What is the formula for collecting gases over water?
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Ptotal = Pgas + PH2O
PH2O value found through a table |
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Who developed the Kinetic-Molecular Theory and what are the postulates that make it up?
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developed by Rudolf Clausius in 1857
1. gases made up of molecules in constant random motion 2. combined volume of gas molecules is negligible to the total volume of the gas 3. attractive and repulsive forces between molecules are negligible 4. energy transferred between collisions, the average kinetic energy, stays the same, elastic collisions 5. the average kinetic energy is proportional to the absolute temperature |
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What is Graham's Law of Effusion and what formula describes it?
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effusion rate of a gas is inversely proportional to the molar mass
a lighter gas effuses more quickly Rate1 / Rate2 = square root of (Mass2 / Mass 1) |
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What are some characteristics of gases?
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The volume of a gas is the same as the container
Gases are highly compressible Gases always mix in homogeneous mixtures Gas particles move faster than solids and liquids Gases have lower densities than solids and liquids Gas volume is affected by pressure, temperature, and number of moles of gas Gases consist of monotonic, diatomic, or small molecular weight molecules |
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What are the pressure conversions?
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1 atm = 760 mmHg = 760 torr = 101.325 kPa
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What is pressure, and where do gases exert pressure?
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P = F/A
gases exert pressure on any organism |
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What is Gay-Lussac's Law, and what formula is used to represent it?
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temperature and pressure are directly proportional
V/T = constant V1/T1 = V2/T2 |
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What is the combined gas law?
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PV/T = constant
P1V1/T1 = P2V2/T2 combination of three gas laws |
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What is diffusion?
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movement from a higher concentration to a lower concentration spontaneously, varies with size and speed of gas, affected by speed and mean free path
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What is effusion?
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the escape of gas molecules through a pinhole sized opening into an evacuated space
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What is the formula for rate of effusion?
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r1/r2 = u1/u2
u= sqrt(3RT/M) closely related to root mean speed, rms = u |
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What is the Van der Waals Equation, and when is this formula used?
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P= nRT/V-nb - (n^2a/V^2)
a, b constants from a table used when the gas is not ideal |
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When are gases not ideal the most?
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at high temperature- volume is lower, actual volume of molecules becomes a factor
at lower temperatures- attractive forces cause pressure to be lower than is ideal |
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What are the assumptions in the Kinetic Molecular Theory?
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1. actual volumes of molecules are negligible
2. attractive/repulsive forces are negligible |
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What is the formula for finding the density of a gas?
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d = MP/RT
at same pressure and temperature, d1/d2 = M1/M2 |
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How would you measure gas pressure with a manometer?
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Pgas = Patm + Ph
Ph is the difference in heights of mercury in two arms of manometer |
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What is the mean free path?
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the average distance traveled by a molecule between collisions, varies with pressure
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What is Avogadro's Hypothesis?
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equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
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What is STP?
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standard temperature and pressure
273 K and 1 atm |
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What is the formula for average kinetic energy of gas molecules?
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E = 1/2mu^2
u= root mean square speed m= mass of the molecule |
